Calculate the osmotic pressure of a solution containing 19.35 mg of hemoglobin in 14.5 mL of solution at 23 °C. The molar mass of hemoglobin is 6.5×10^4 g/mol. Assume the solution behaves ideally. (R = 0.0821 L·atm/mol·K)

Using the van’t Hoff factors in Table 13.9, calculate the mass of solute required to make each aqueous solution: a. a sodium chloride solution containing 1.50 * 10^2 g of water that has a melting point of -1.0 °C; b. 2.50 * 10^2 mL of a magnesium sulfate solution that has an osmotic pressure of 3.82 atm at 298 K; c. an iron(III) chloride solution containing 2.50 * 10^2 g of water that has a boiling point of 102 °C.

Is the question asking for the calculation of the van’t Hoff factor (i) for KBr at a given concentration, based on the provided osmotic pressure, correct?

A compound is found to have a molar mass of 598 g/mol. If 35.8 mg of the compound is dissolved in enough water to make 175 mL of solution at 25°C, what is the osmotic pressure of the resulting solution? (Assume ideal behavior and R = 0.0821 L·atm/mol·K)

Calculate the osmotic pressure of a solution containing 18.95 mg of hemoglobin in 16.6 mL of solution at 18 °C. The molar mass of hemoglobin is 6.5×10^4 g/mol. Express your answer in atmospheres.

Calculate the osmotic pressure of a solution containing 19.45 mg of hemoglobin in 16.8 mL of solution at 18 °C. The molar mass of hemoglobin is 6.5×10^4 g/mol. Assume the solution behaves ideally and use R = 0.0821 L·atm/mol·K.

Calculate the osmotic pressure of a solution made by dissolving 14.65 g of sucrose (C12H22O11) in water to make 275 mL of solution at 43°C. (R = 0.0821 L·atm/mol·K, Molar mass of sucrose = 342.3 g/mol)

What is the osmotic pressure of a solution containing 14 g of urea (H₂NCONH₂) in 300 mL of water at 217°C? (R = 0.0821 L·atm/mol·K)

What is the osmotic pressure (in atm) of an aqueous solution that contains 162.1 g of glucose (C₆H₁₂O₆) in 1.50 L of solution at 295 K? (R = 0.0821 L·atm/mol·K, Molar mass of glucose = 180.18 g/mol)